Question

For a phase change, H = 2 kJ/mol and S = 0.017 kJ/(K-mol). What are
G and the spontaneity of the phase change at 500 K?
A. G=-6.5 kJ; nonspontaneous
B. G= 10.5 kJ; spontaneous
C. G= 10.5 kJ; nonspontaneous
D. G=-6.5 kJ; spontaneous

Answer 1

The reaction has a change in free energy of -6.5 kJ and is spontaneous Option D.

What is a spontaneous reaction?

The term spontaneous reaction refers to a reaction that occurs with n external input of energy. We know that a spontaneous reaction is one in which the value of the change in free energy is negative. If the change in the free energy is positive then the reaction is nonspontaneous.

If the value of the change in free energy is zero then it follows that the reaction has attained equilibrium.

Now;

ΔG = ΔH - TΔS

ΔH = 2 kJ/mol

T =  500 K

ΔS =  0.017 kJ/(K-mol)

When we substitute values;

ΔG = 2 kJ/mol - (500 K * 0.017 kJ/(K-mol))

ΔG = -6.5 kJ

It the follows that the reaction has a change in free energy of -6.5 kJ and is spontaneous Option D.

Learn more about spontaneous reaction:https://brainly.com/question/13790391

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